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chapters 1-2 review Name: __ Objectives:
Describe the states and types of matter and the history of the periodic table
Interpret and use atomic symbols, the periodic table, and chemical formulas
Describe a critical skill of scientists
Distinguish chemical changes and properties from physical changes and properties
Use the scientific method
Distinguish mass from weight
Use conversion factors in solving mathematical problems
Identify significant figures in measurements
Distinguish between accuracy and precision in experimental results
Use density in lab results
Multiple choice: choose the best answer
1.
What are two of the properties of non-metallic elements?
A)
They conduct both heat and electricity.
B)
They conduct heat but not electricity.
C)
They conduct neither heat nor electricity.
D)
They conduct electricity but not heat.
2.
The atomic symbol that corresponds to the name silver is
A)
Au
B)
Ag
C)
Si
D)
Sb
3.
Which series of elements are metalloids?
A)
tungsten, silicon, and gallium
B)
tungsten, sulfur, and silver
C)
germanium, antimony, and boron
D)
gallium, germanium, and antimony
4.
The atomic symbols that correspond to sulfur, antimony, and silicon are
A)
S, Sb, and Si
B)
Se, Sb, and Si
C)
S, Se, and Si
D)
S, Sb, and Se
5.
What is the simplest unit of an ionic compound?
A)
a molecule
B)
an element
C)
a formula unit
D)
an ion
6.
Why are different materials separated by chromatography?
A)
Each material has a slightly different color than the others in the mixture.
B)
Each material moves at a slightly different speed from others in the mixture.
C)
Each material is a different compound in the mixture.
D)
Each material moves at a similar speed to others in the mixture.
7.
Which atomic symbols correspond to hydrogen, mercury, and helium, in that order?
A)
Hy, Hg, and He
B)
H, Me, and He
C)
H, Hg, and Hl
D)
H, Hg, and He
8.
What element name corresponds to the elemental symbol Sb?
A)
antimony
B)
lead
C)
tin
D)
arsenic
9.
What is the name that corresponds to the elemental symbol W?
10.
The smallest unit of an element is an atom.
A)
True
B)
False
11.
Write the formula for sodium chloride, which has 1 atom of sodium and 1 of chlorine.
A)
NaCl
B)
NaCl2
C)
Na2Cl
D)
Na2Cl2
12.
The symbol Cu represents what element?
13.
Which of the following elements are metals?
A)
Mg, K, and S
B)
Mg, K, and Na
C)
Mo, O, and Na
D)
Mg, K, and F
14.
Forensic chemistry can be used to determine the composition of
A)
drugs
B)
explosives
C)
both of the above
D)
neither of the above
15.
Pure substances
A)
have a uniform composition and cannot be separated by physical methods
B)
are always elements
C)
are solids in most cases
D)
have a uniform composition that can be separated by physical methods
16.
What is the volume of a chemical sample with a density of 0.982 g/mL and a mass of 6.14 g?
A)
5.16 mL
B)
0.160 mL
C)
6.25 mL
D)
6.03 mL
17.
How dense is a material with a volume of 13.0 mL and a mass of 14.2g?
A)
1.09 g/mL
B)
1.20 g/mL
C)
0.92 g/mL
D)
27.2 g/mL
18.
How many significant figures does the number 23.500 have?
19.
What is the volume of a sample with a density of 1.23 g/mL and a mass of 0.023 kg?
A)
18.7 mL
B)
0.0187 mL
C)
1.21 mL
D)
283 mL
20.
Which of the following represent three measurements that are the least precise?
A)
2.34, 2.40, and 2.37
B)
14.2, 14.1, and 14.3
C)
3.45, 45.3, and 13.1
D)
35.2, 35.5, and 35.4
21.
How many centimeters are there in 2.54 in.?
A)
6.45
B)
1.00
C)
5.08
D)
15.48
22.
If a true value for the mass of a sample is 1,300 g, which of the following is the most accurate?
A)
1,200 g
B)
1,295 g
C)
1,350 g
D)
1,310 g
23.
If a true value for the mass of a sample is 0.100 g, which of the following is the most accurate?
A)
0.105 g
B)
0.099 g
C)
0.104 g
D)
0.093 g
24.
What is the mass of a material with a density of 2.22 g/mL and a volume of 2.30 mL?
A)
0.51g
B)
5.11g
C)
0.96g
D)
9.65g
25.
A liquid sample with a density of 5.25 g/mL and a mass of 1.11 g has what volume?
A)
5.83 mL
B)
0.211 mL
C)
4.73 mL
D)
4.14 mL
26.
How many milliliters are in 0.468 L?
A)
468
B)
46.8
C)
4.68
D)
0.0468
27.
What is a characteristic of a chemical change?
A)
a substance melts or freezes
B)
a material evaporates
C)
neither of the above
D)
both of the above
28.
How many significant figures are there in the number 12,100?
29.
What is the density of a white powder with a mass of 12.5 g and a volume of 10.3 mL?
30.
Convert 830 mL to L:
31.
How dense is a powdered material with a mass of 9.8 g and a volume of 1.2 mL?
32.
Which of the following elements are non-metals: chromium, fluorine, oxygen, chlorine, francium, and/or copper?
33.
What elements are present, and how many atoms of each are in the compound KMnO4?
34.
Explain distillation and its purpose in chemistry.
35.
Describe the properties and distinguish between metals, nonmetals, and metalloids.
36.
Define matter. Describe the two types of matter and how to differentiate them.
Chapter 3 final exam review Objectives:
Distinguish between the early schools of thought on the nature of the atom.
Know the effects of politics on the development of the atomic theory
Know and understand Dalton’s atomic theory
Know the subatomic particles and their characteristics
Know and understand the modern model of the atom
Describe the behavior of light and carry out calculations.
Define and describe isotopes and calculate the weighted atomic mass of an element.
Understand the atomic emission spectra.
Write electron configurations.
Multiple choice: choose the best answer
1.
What is the full electron configuration for arsenic?
A)
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2
B)
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3
C)
1s2 2s2 2p6 3s2 3p6 4s2 3d11 4p2
D)
1s2 2s2 2p6 3s2 3p6 4s2 3d10
2.
The isotope of cobalt with the symbol 5927Co has how many electrons?
A)
33
B)
32
C)
59
D)
27
3.
Which isotope of neon is the major one?
A)
20
B)
21
C)
22
D)
23
4.
Uranium metal, made only of uranium atoms, has how many protons in each atom?
A)
90
B)
238
C)
235
D)
92
5.
What is a photon?
A)
excess energy absorbed by a proton
B)
excess energy emitted from a neutron
C)
excess energy absorbed by an electron
D)
excess energy emitted from an electron
6.
What is the full electron configuration for nitrogen?
A)
1s2 2s2 2p3
B)
1s2 2s2 2p6 3s2
C)
1s2 2s2 2p4 3s2
D)
1s2 2s2 2p6
7.
An electron configuration of 1s2 2s2 2p6 3s2 3p6 4s2 represents which element?
A)
Mg
B)
Ca
C)
Sr
D)
None, the configuration is incorrect for any element.
8.
The electron configuration 1s2 2s2 2p1 is correct for which element?
A)
He
B)
Be
C)
C
D)
B
9.
The isotope of osmium with the symbol 19075Os has how many protons?
A)
75
B)
190
C)
115
D)
None of the above
10.
How many neutrons does uranium – 235 contain?
A)
92
B)
140
C)
143
D)
235
11.
When an element has Z = 31 and 39 neutrons, what element and isotope is it?
A)
3170Ga
B)
3170Yb
C)
7031Ga
D)
7031Yb
12.
When Lavoisier heated mercury (II) oxide, what were his products?
A)
mercury gas and oxygen liquid
B)
mercury oxide and oxygen gas
C)
mercury gas and oxygen gas
D)
mercury liquid and oxygen gas
13.
Which element has the electron configuration 1s2 2s2 2p5?
A)
neon
B)
oxygen
C)
chlorine
D)
fluorine
14.
What is the orbital of an electron?
A)
a loop-like planetary trajectory with the lowest probability of finding the electron
B)
a loop-like planetary trajectory with the highest probability of finding the electron
C)
the region of space with the lowest probability of finding the electron
D)
the region of space with the highest probability of finding the electron
15.
The isotope of cobalt with the symbol 5927Co has how many neutrons?
A)
27
B)
32
C)
59
D)
86
16.
What is different in isotopes of the same element?
17.
Define and describe forensic science.
18.
Define and describe the three states of matter.
19.
Describe the history of the periodic table. Include Mendeleev and Mosely.
20.
Distinguish between accuracy and precision in experimental results.
21.
Distinguish between chemical changes and physical changes as well as chemical properties and physical properties.
22.
Describe the Atomic Theory.
23.
Which element has the electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3?
24.
The full electron configuration for C is
25.
Write the electron configuration of Zn
26.
What is difference between the isotopes of Carbon-12 and Carbon-14?
27.
Explain how atoms produce light.
28.Calculate the frequency of a photon with a wavelength of 900nm. 29.Calculate the wavelength in nm of a photon with a frequency of 1.66x1015 Hz. 30.Calculate the energy of a photon with a frequency of 2.25 x1014 Hz. 31.Calculate the energy of a photon with a wavelength of 650nm. 32.In a reaction in which 54.0 g of HgO is heated, liberating 43.0 g of mercury, how much oxygen must also have been produced? Give a brief description of each of the scientist's discoveries or contributions: 33.a. Dalton b Rutherford c. Chadwick d. Thompson e. Proust f. Gassendi g. Lavosier h. Democritus i. Goldstein chapter 4 part I review Objectives:
Describe how Avogadro’s Number is related to a mole of any substance and use it in conversions.
Calculate the mass of a mole of any substance.
Use molar mass to convert between mass and moles of a substance.
Learn the different types of reactions and how to predict products.
Learn how to use mole to mole ratios to calculate quantities of reactants needed or amount of product made.
Identify the limiting reactant.
Calculate theoretical yield based on limiting reactant
1.Name two different things that 1 mole is equal to. 2.Distinguish between a combustion reaction, a neutralization reaction, and a precipitation reaction. 3.What is a salt? 4.What is a mole to mole ratio and when is it used? 5.Define limiting reactant and theoretical yield. 6.Balance the following equations: a.S2+O2®SO3 b.NaF +Mg(NO3)2® NaNO3+MgF2 7.Write a balanced equation for the following reaction: magnesium and copper (I) nitrate form copper and magnesium nitrate 8.Identify the following reactions as precipitation, combustion, or neutralization. a.Ca(OH)2 aq + HNO3 aq→Ca(NO3)2 aq + H2O l b.AgNO3 aq + NaCl aq → AgCl s + NaNO3 aq c.C2H5OH l + O2 g → H2O l + CO2 g 9.Predict the products of the following a. the combustion of propane (C3H8) and oxygen c.the neutralization of HCl and RbOH 10.What is the mass in grams of 2.5 moles of gold? 11.What is the molar mass of Al2(SO4)3? 12.What is the mass in grams of 2.50 moles of MgO? How many particles? 13.A sample has 15.7 g of vanadium. How many atoms are in this sample? 14.How many moles are in 8.29 g of water? 15.How many particles are in 141.5 g of Al2(SO4)3? 16.What is the theoretical yield in grams of water if 12.5 g of CH3OH are completely consumed, according to the equation: 2CH3OH + 3 O2 ® 2CO2 + 4 H2O 17.How many grams of phosphorous are needed to react completely with 14.0 g of Al when aluminum reacts with phosphorous to form aluminum phosphide? 18.If 42.0 g of sodium and 32.0 g of oxygen are mixed according to the equation 4 Na + O2 ® 2 Na2Owhat is the theoretical yield and which is the limiting reagent? 19.Calcium reacts with hydrogen chloride to form calcium chloride and hydrogen gas. What is the theoretical yield in grams of calcium chloride and which is the limiting reactant when 55.0 g of calcium is mixed with 35.5 g HCl?
Chapter 12 final exam review Objectives:
Know the history of radioactivity
Discuss the processes of radioactivity and radioactive decay and know the risks.
Characterize alpha, beta, and gamma radiation in terms of composition and penetrating power and balance radioactive decay reactions.
Understand half lives.
Compare nuclear fission and nuclear fusion and comment on their potential as sources of energy.
Describe methods of detecting radiation.
List some applications of radioisotopes in research, medicine, and the military.
Explain nuclear transmutation.
1.
Balance the following: a.24294Pu ®23892U+_
b.Np-237 releases an alpha and a gamma particle.
c.23490Th ®0-1e +__
2.
I-131 has a half life of 8 days. How much do you have after 6 half lives if you start with 120g? How many days does it take to complete 6 half lives?
3. Name and give the characteristics of the three radiactive particles.
4. What is a dirty bomb?
5.Describe Henri Becquerel’s experiment and its importance to the discovery of radiactivity.
6. List Marie Curie’s scientific accomplishments.
7. What is radiation sickness?
8. Name the three parts of a nuclear power plant and explain the function of each one.
9. Discuss fission and fusion.
10. What is phosphorescence?
14.You have been given an artifact to C-14 date. The half life of C-14 is 5730 years. If the artifact was at day 0 it would have 425g of carbon. a.)In the table below, fill in the grams and years for 6 half lives. b.)Draw a graph representing the decay of C-14 on the graph below. c.)Based on the graph determine the age of the artifact if it has 48.0g of C-14.
Final Exam review for fall semester
please note that the subscripts and superscripts are not formatted - they are in the regular text.chapters 1-2 review
Name: __
Objectives:
Multiple choice: choose the best answer
Chapter 3 final exam review
Objectives:
Multiple choice: choose the best answer
28. Calculate the frequency of a photon with a wavelength of 900nm.
29. Calculate the wavelength in nm of a photon with a frequency of 1.66x1015 Hz.
30. Calculate the energy of a photon with a frequency of 2.25 x1014 Hz.
31. Calculate the energy of a photon with a wavelength of 650nm.
32. In a reaction in which 54.0 g of HgO is heated, liberating 43.0 g of mercury, how much oxygen must also have been produced?
Give a brief description of each of the scientist's discoveries or contributions:
33. a. Dalton
b Rutherford
c. Chadwick
d. Thompson
e. Proust
f. Gassendi
g. Lavosier
h. Democritus
i. Goldstein
chapter 4 part I review
Objectives:
1. Name two different things that 1 mole is equal to.
2. Distinguish between a combustion reaction, a neutralization reaction, and a precipitation reaction.
3. What is a salt?
4. What is a mole to mole ratio and when is it used?
5. Define limiting reactant and theoretical yield.
6. Balance the following equations:
a. S2 + O2 ® SO3
b. NaF + Mg(NO3)2 ® NaNO3 + MgF2
7. Write a balanced equation for the following reaction:
magnesium and copper (I) nitrate form copper and magnesium nitrate
8. Identify the following reactions as precipitation, combustion, or neutralization.
a. Ca(OH)2 aq + HNO3 aq →Ca(NO3)2 aq + H2O l
b. AgNO3 aq + NaCl aq → AgCl s + NaNO3 aq
c. C2H5OH l + O2 g → H2O l + CO2 g
9. Predict the products of the following
a. the combustion of propane (C3H8) and oxygen
c. the neutralization of HCl and RbOH
10. What is the mass in grams of 2.5 moles of gold?
11. What is the molar mass of Al2(SO4)3?
12. What is the mass in grams of 2.50 moles of MgO? How many particles?
13. A sample has 15.7 g of vanadium. How many atoms are in this sample?
14. How many moles are in 8.29 g of water?
15. How many particles are in 141.5 g of Al2(SO4)3?
16. What is the theoretical yield in grams of water if 12.5 g of CH3OH are completely consumed, according to the equation: 2CH3OH + 3 O2 ® 2CO2 + 4 H2O
17. How many grams of phosphorous are needed to react completely with 14.0 g of Al when aluminum reacts with phosphorous to form aluminum phosphide?
18. If 42.0 g of sodium and 32.0 g of oxygen are mixed according to the equation
4 Na + O2 ® 2 Na2O what is the theoretical yield and which is the limiting reagent?
19. Calcium reacts with hydrogen chloride to form calcium chloride and hydrogen gas. What is the theoretical yield in grams of calcium chloride and which is the limiting reactant when 55.0 g of calcium is mixed with 35.5 g HCl?
Chapter 12 final exam review
Objectives:
a. 24294Pu ® 23892U +_
b. Np-237 releases an alpha and a gamma particle.
c. 23490Th ® 0-1e +__
3. Name and give the characteristics of the three radiactive particles.
4. What is a dirty bomb?
5. Describe Henri Becquerel’s experiment and its importance to the discovery of radiactivity.
6. List Marie Curie’s scientific accomplishments.
7. What is radiation sickness?
8. Name the three parts of a nuclear power plant and explain the function of each one.
9. Discuss fission and fusion.
10. What is phosphorescence?
14. You have been given an artifact to C-14 date. The half life of C-14 is 5730 years. If the artifact was at day 0 it would have 425g of carbon.
a.) In the table below, fill in the grams and years for 6 half lives.
b.) Draw a graph representing the decay of C-14 on the graph below.
c.) Based on the graph determine the age of the artifact if it has 48.0g of C-14.
Years
0
Grams
425g